Thermodynamics And Calorimetry Lab Report
Wissam Kamaleddine
CHM 1120
Stanley Ngeyi
February 25,2012
Thermodynamics/Calorimetry
Introduction: Thermochemistry investigates the relationship between chemical reactions and energy changes involving heat. The amount of heat generated or absorbed in a chemical reaction can be studied using a calorimeter.
Purpose: The purpose of this laboratory was to determine the heat capacity of the calorimeter, and to understand thermodynamics/calorimetry by applying the calorimetry equation, Heat lost=Heat gained. We will use calorimetry to determine the heat involved when ammonium chloride, NH4Cl, dissolves in water. In this experiment our attention is focused on the reaction between ammonia and hydrogen chloride: NH3 + HCl --> NH4Cl …show more content…
Results Part B: Heat of dissociation of NH4Cl(s)
Pasted Graphic 1.pdf
Calculations:
(a) The change in temperature for the solution and the calorimeter as determined from the figure is: ^T=Tf-Ti=18.0 deg. C - 25.0 deg. C = -7.0 deg. C
(b) Heat of reaction q=heat lost by solution + heat lost by
CHM 1120
Stanley Ngeyi
February 25,2012
Thermodynamics/Calorimetry
Introduction: Thermochemistry investigates the relationship between chemical reactions and energy changes involving heat. The amount of heat generated or absorbed in a chemical reaction can be studied using a calorimeter.
Purpose: The purpose of this laboratory was to determine the heat capacity of the calorimeter, and to understand thermodynamics/calorimetry by applying the calorimetry equation, Heat lost=Heat gained. We will use calorimetry to determine the heat involved when ammonium chloride, NH4Cl, dissolves in water. In this experiment our attention is focused on the reaction between ammonia and hydrogen chloride: NH3 + HCl --> NH4Cl …show more content…
Results Part B: Heat of dissociation of NH4Cl(s)
Pasted Graphic 1.pdf
Calculations:
(a) The change in temperature for the solution and the calorimeter as determined from the figure is: ^T=Tf-Ti=18.0 deg. C - 25.0 deg. C = -7.0 deg. C
(b) Heat of reaction q=heat lost by solution + heat lost by